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Lanthanide and actinide series do not start with lanthanum and actinium explain?
Lets take the Lanthanides as an example. Lanthanum has its 5d sublevel filled before its 4f, even though the 4f is lower in energy and should, by the Aufbau Principle, be filled first. However, this is an exception because it happens to be the most stable configuration. It has one electron in the 5d sublevel and none in the 4f, and since it has no "f" electrons, it cannot be part of the f-bar's upper row (the Lanthanide series). The Lanthanides themselves will each also have one electron in the 5d sublevel, and the first element will also have one in the 4f sublevel. This trend will continue for all 14, and thus the 4f sublevel is filled. Hafnium, the element immediately after the last Lanthanide, will resume filling the 5d sublevel as normal, with two electrons in it and a completely filled 4f sublevel. The anomaly does not really change much; after all, if the valence electron in Lanthanum were not in the 5d sublevel and instead in the 4f, it would start off the Lanthanide series, there would be 14, and it would simply end one element before it normally does. The numbers all add up, in any case, and this is the natural order of things. For Actinides, replace the word Lanthanum with Actinium, Hafnium with Darmstadtium, 5d with 6d, and 4f with 5f. Everything works out perfectly; all the confusion is just caused by the stubborn little electron who doesn't want to be the first f-block element (and so he moves up into 5d, and stays there while the others take their appropiate places, which are moved one up thanks to his desire to maintain stability).
What sublevel is neon?
Neon is located in the p sublevel.
What is the atomic sublevel with the next highest energy after 4p?
The next highest energy atomic sublevel after 4p is the 5s sublevel. In the electron configuration of an atom, energy levels increase with increasing principal quantum number (n), so the 5s sublevel is higher in energy than the 4p sublevel.
This element has two electrons in the 1st sublevel and 4 electrons in the 2nd sublevel?
CARBON
Where are the electrons being added from in the 4f orbitals?
Electrons are added to the 4f orbitals from the 5d orbitals in the lanthanide and actinide series of elements. The 4f orbitals are filled after the 5d orbitals are filled due to the overlap in energy levels, leading to the stability of the 4f electrons in these elements.
Which energy sublevel is being filled by the elements Ce to Lu?
The energy sublevel being filled by the elements Ce to Lu is the 4f sublevel. These elements are part of the lanthanide series and have their outermost electrons entering the 4f orbital.
What is the highest sublevel electrons in the element Promethium an f block element occupy?
The highest sublevel that Promethium can have is 4f. It is possible for 14 electrons to be placed around Promethium, since the elements in this sublevel each have 7 orbitals.
Which set of elements has electrons added to the 4f sublevel as the atomic number increases?
The set of elements that has electrons added to the 4f sublevel as the atomic number increases are the lanthanide series elements, from cerium (Z = 58) to lutetium (Z = 71). The 4f sublevel can hold up to 14 electrons per element, hence as we move across this series, electrons are successively added to the 4f sublevel.
How many orbitals are found in the f sublevel?
There are 7 orbitals in the f sublevel. These orbitals are designated as 4f, 5f, 6f, 7f, 8f, 9f, and 10f.
How many electrons can occupy the 4f sublevel?
The elements in period 4 that have electrons in the 3d sublevel are elements 21 - 36. Refer to the Related Links for a printable periodic table that includes electron configurations.
How many 4f orbitals are in an atom?
some atoms have 5, some have none. the max is 5
Which sublevel has 7 orbitals?
I try to answer your question sub shell no. of orbitals s 1 p 3 d 5 f 7 Hope you will be satisfied
Where does the final electron in inner transition metals enter?
The final electron in inner transition metals typically enters the 4f or 5f orbitals. These orbitals are part of the inner electron shells and are responsible for the unique chemical properties of inner transition metals.
Lanthanide and actinide series do not start with lanthanum and actinium explain?
Lets take the Lanthanides as an example. Lanthanum has its 5d sublevel filled before its 4f, even though the 4f is lower in energy and should, by the Aufbau Principle, be filled first. However, this is an exception because it happens to be the most stable configuration. It has one electron in the 5d sublevel and none in the 4f, and since it has no "f" electrons, it cannot be part of the f-bar's upper row (the Lanthanide series). The Lanthanides themselves will each also have one electron in the 5d sublevel, and the first element will also have one in the 4f sublevel. This trend will continue for all 14, and thus the 4f sublevel is filled. Hafnium, the element immediately after the last Lanthanide, will resume filling the 5d sublevel as normal, with two electrons in it and a completely filled 4f sublevel. The anomaly does not really change much; after all, if the valence electron in Lanthanum were not in the 5d sublevel and instead in the 4f, it would start off the Lanthanide series, there would be 14, and it would simply end one element before it normally does. The numbers all add up, in any case, and this is the natural order of things. For Actinides, replace the word Lanthanum with Actinium, Hafnium with Darmstadtium, 5d with 6d, and 4f with 5f. Everything works out perfectly; all the confusion is just caused by the stubborn little electron who doesn't want to be the first f-block element (and so he moves up into 5d, and stays there while the others take their appropiate places, which are moved one up thanks to his desire to maintain stability).
What in the electrons are being added to the 4f orbitals?
If the valence electrons are being added to the 4f orbitals, that means the element is lanthanides or actinides which further proves that the element is a heavy element and a member of f -block.
What is the correct electron configuration for an element with 5 electrons in the 3d energy sublevel?
The correct electron configuration would be 3d5 as each orbital in the 3d sublevel can hold up to 2 electrons, and we have 5 electrons to place in this sublevel.
What electron configuration of outer sublevels is the most stable?
The electron configuration of the 4f energy sublevel is the most stable is 4f to the 14th power. The electron configuration of outer sublevels that are most stable is 4d up to the 5.5s up to the 1st power.
